Single Choice

Which of the following have the largest ionic size?

A$$F^-$$
B$$O^{2-}$$
Correct Answer
C$$Na^+$$
D$$Mg^{2+}$$

Solution

All species are isoelectronic. They have 10 electrons.

$$\displaystyle O^{2-}$$ has a least nuclear charge ( due to lowest atomic number) and hence has the largest ionic size as few positive charges are attracting more negative charges.

The correct order of ionic size:
$$O^{2-} > F^- > Na^+ > Mg^{2+}$$

Hence, option B is correct.

SIMILAR QUESTIONS

Chemical Bonding

Which of the following arrangements represents the increasing order (smallest to largest) of ionic radii of the given species $$O^{2-}, S^{2-}, N^{3-}, P^{3-}$$?

Chemical Bonding

The ionic radii (in $$\mathring{A}$$) of $$N^{3-}$$, $$O^{2-}$$ and $$F^{-}$$ are respectively :

Chemical Bonding

The increasing order of the ionic radii of the given isoelectronic species is:

Chemical Bonding

The correct order of decreasing ionic radius among the following anions would be:

Chemical Bonding

The species $$Ar, K^+$$ and $$Ca^{2+}$$ contain the same number of electrons. In which order do their radii increase?

Chemical Bonding

What do you understand by isoelectronic species? Name a species that will be isoelectronic with each of the following atoms or ions. (i) F$$\displaystyle ^{-}$$ (ii) Ar (iii) Mg$$\displaystyle ^{2+}$$ (iii) Rb$$\displaystyle ^{+}$$

Chemical Bonding

The size of isoelectronic species $$F\displaystyle ^{-}$$, $$Ne$$ and $$Na\displaystyle ^{+}$$ is affected by :

Chemical Bonding

$$K^{+}$$ and $$Cl^{-}$$ ions are isoelectronic. Which of the following statements is not correct?

Chemical Bonding

Which one of the following groups represents a collection of isoelectronic species? (At. nos.: Cs-55, Br-35)

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